A certain reaction is zero order in reactant A and second order in reactant B. What happens to the reaction rate when the concentrations of both reactants are doubled?

Choose one answer.

	a. The reaction rate remains the same.
	b. The reaction increases by a factor of two.
	c. The reaction increases by a factor of four.
	d. The reaction increases by a factor of eight.

Question 2

A rate law relates which of the following?

Choose one answer.

	a. Reaction rate and temperature
	b. Reaction rate and concentration
	c. Temperature and concentration
	d. Energy and concentration

Question 3

Determine the overall balanced equation for a reaction that has the following proposed mechanism. Which of the following is the acceptable rate law?
Step 1: B₂ + B₂ → E₃ + D slow
Step 2: E₃ + A → B₂ + C₂ fast

Choose one answer.

	a. B₂ + B₂ → E₃ + D and R = [B₂]²
	b. A + B₂→ C₂ + D and R = [A] [B₂]²
	c. A + B₂ → C₂ + D and R = [B₂]²
	d. A + B₂→ C₂+ D and R = [E₃] [A]

Question 4

Fill in the blank. A species that changes the rate of a reaction but is neither consumed nor changed in that reaction is a(n) ________________.

Choose one answer.

	a. Catalyst
	b. Activated complex
	c. Intermediate
	d. Reactant

Question 5

If two molecules collide softly, what will most likely happen to the molecules?

Choose one answer.

	a. The molecules will be oriented favorably.
	b. The molecules will not be oriented favorably.
	c. The molecules are likely to react.
	d. The molecules may rebound without reacting.

Question 6

The decomposition of nitrogen dioxide 2 NO₂ → 2 NO + O₂ occurs in a two-step sequence at elevated temperatures. The first step is NO₂ → NO + O. Which of the following accurately predicts the second step that, when combined with the first step, gives the complete reaction?

Choose one answer.

	a. NO₂ + O → NO + O₂
	b. O → NO + O₂
	c. NO₂→ NO
	d. O₂→ NO + 3 O₂

Question 7

To be effective, a collision requires which of the following?

Choose one answer.

	a. Enough energy
	b. Favorable orientation
	c. A reaction mechanism
	d. Both A and B

Question 8

What is the slowest step in a reaction mechanism called?

Choose one answer.

	a. The rate-determining step
	b. The uncatalyzed reaction
	c. The activation step
	d. None of the above

Question 9

Which of the following statements most accurately describes the energy of the activated complex also called transition state?

Choose one answer.

	a. The transition state is lower than the energy of the reactants but higher than the energy of the products.
	b. The transition state is lower than the energy of both the reactants and the products.
	c. The transition state is higher than the energy of the reactants but lower than the energy of the products.
	d. The transition state is higher than the energy of both the reactants and the products.

Question 10

Fill in the blank. The sequence of steps that occurs in a reaction process is called the _____________.

Choose one answer.

	a. Order of the reaction
	b. Reaction mechanism
	c. Overall reaction
	d. Rate law

Question 11

A silver chloride solution is prepared with the following ion concentrations [Ag⁺] = 1.0 x 10^-6 M and [Cl^-] = 1.0 x 10^-2 M. If K_sp for AgCl = 1.8 x 10^-10, then which of the following is true?

Choose one answer.

	a. A precipitate will form.
	b. A precipitate will not form.
	c. The system is at equilibrium.
	d. None of the above

Question 12

Acetic acid is a weak electrolyte, because it does which of the following?

Choose one answer.

	a. Becomes miscible with water
	b. Forms hydronium and hydroxide ions in aqueous solution
	c. Lowers the freezing point of water
	d. Ionizes only slightly in aqueous solution

Question 13

How can one prepare a 1.00 L of a 0.125 M H₂SO₄ solution?

Choose one answer.

	a. Dilute 36.0 mL of 1.25 M H₂SO₄ to a volume of 1.00 L.
	b. Dilute 20.8 mL of 6.00 M H₂SO₄ to a volume of 1.00 L.
	c. Add 950. mL of water to 50.0 mL of 3.00 M H₂SO₄.
	d. Add 500. mL of water to 500. mL of 0.500 M H₂SO₄.

Question 14

How many grams of Na₃PO₄ are there in 500. mL of a 0.250 M solution of Na₃PO₄ (molar mass = 163.94 g/mol)?

Choose one answer.

	a. 2.05 g
	b. 20.5 g
	c. 0.125 g
	d. 0.168 g

Question 15

Solution A contains 0.1 mol of sucrose, C₁₂H₂₂O₁₁, dissolved in 500 g of water. Solution B contains 0.1 mol of sodium chloride, NaCl, in 500 g of water. Which of the following statements about these solutions is true?

Choose one answer.

	a. Both solutions have the same vapor pressure.
	b. Solution A would boil at a higher temperature than solution B would.
	c. Solution A would freeze at higher temperature than solution B would.
	d. Both solutions would boil at the same temperature.

Question 16

The solubility of AgCl is 1.22 x 10^-8 mol/L. What is the value of K_sp for AgCl?

Choose one answer.

	a. 1.1 x 10⁻⁴
	b. 1.2 x 10⁻⁸
	c. 5.7 x 10⁻²
	d. 1.5 x 10⁻¹⁶

Question 17

To make a water-soluble salt using the silver cation, Ag+, what anion should be chosen?

Choose one answer.

	a. NO₃⁻
	b. CO₃²⁻
	c. Cl⁻
	d. PO₄³⁻

Question 18

Use the solubility rules. Which salt is insoluble in water?

Choose one answer.

	a. NaBr
	b. NH₄Cl
	c. FeS
	d. (NH₄)₂S

Question 19

Use the solubility rules. Which salt is soluble in water?

Choose one answer.

	a. Fe(OH)₃
	b. AgCl
	c. CaCl₂
	d. BaSO₄

Question 20

What is the balanced, net ionic equation for the reaction of nickel(II) chloride and sodium phosphate to give nickel(II) phosphate and sodium chloride?

Choose one answer.

	a. 2 Na₃PO₄(aq) + 3 NiCl₂(aq) → Ni₃(PO₄)₂(s) + 6 NaCl(aq)
	b. 2 Na₃PO₄(aq) + 3 NiCl₂(aq) → Ni₃(PO₄)₂(aq) + 6 NaCl (aq)
	c. 2 PO₄³⁻(aq) + 3 Ni²⁺(aq) → Ni₃(PO₄)₂(s)
	d. Na⁺(aq) + Cl⁻(aq) → NaCl(aq)

Question 21

What is the balanced, net ionic equation for the reaction of aluminum sulfate with sodium hydroxide?

Choose one answer.

	a. Al₂(SO₄)₃(aq) + 6 NaOH(aq) → 2 Al(OH)₃(s) + 3 Na₂SO₄(aq)
	b. Al³⁺(aq) + 3 OH⁻(aq) → Al(OH)₃(s)
	c. Al₂(SO₄)₃(aq) + 6 NaOH(aq) → 2 Al(OH)₃(aq) + 3 Na₂SO₄(s)
	d. 2 Na⁺(aq) + SO₄²⁻(aq) → Na₂SO₄(s)

Question 22

What is the correct expression for the solubility product constant, K_sp, for FePO₄?

Choose one answer.

	a. K_s_p = [Fe³⁺] / [PO₄³⁻]³
	b. K_s_p = [Fe³⁺][P⁵⁻][O²⁻]³
	c. K_s_p = [Fe³⁺][PO₄³⁻]
	d. K_s_p = [Fe³⁺][PO₄³⁻] / [FePO₄]

Question 23

What is the molality of a 0.907 M Pb(NO₃)₂ solution? (Molar mass of Pb(NO₃)₂ = 331.2 g/mol; density of the solution = 1.252 g/mL.)

Choose one answer.

	a. 0.953 m
	b. 0.724 m
	c. 0.907 m
	d. 1.98 m

Question 24

What is the molality of a solution containing 5.67 g glucose, C₆H₁₂O₆, dissolved in 25.2 g of water? (Molar mass of C₆H₁₂O₆ = 180.2 g/mol.)

Choose one answer.

	a. 0.00125 m
	b. 0.225 m
	c. 1.25 m
	d. 0.762 m

Question 25

What is the molarity of a 0.273 m KCl? (Molar mass of KCl = 74.6 g/mol; density of the solution = 1.011 g/L.)

Choose one answer.

	a. 20.6 M
	b. 1.0 M
	c. 0.273 M
	d. 0.271 M

Question 26

What is the new concentration of a nitric acid made by diluting 50. mL of a 12.0 M solution to 250. mL?

Choose one answer.

	a. 2.4 M
	b. 60. M
	c. 10. M
	d. 24 M

Question 27

What is the total concentration of ions in a 0.0360 M solution of Na₃PO₄?

Choose one answer.

	a. 0.108 M
	b. 0.144 M
	c. 0.0360 M
	d. 0.0720 M

Question 28

What volume in mL of 0.453 M NaCl solution contains 25.0 g of NaCl (molar mass = 58.5 g/mol)?

Choose one answer.

	a. 193 mL
	b. 1000 mL
	c. 943 mL
	d. 453 mL

Question 29

Which of the following is NOT a colligative property?

Choose one answer.

	a. Molality
	b. Vapor-pressure lowering
	c. Boiling-point elevation
	d. Osmotic pressure

Question 30

Which one of the following compounds is a nonelectrolyte when dissolved in water?

Choose one answer.

	a. Sodium chloride
	b. Calcium chloride
	c. Copper sulfate
	d. Sugar

Question 31

A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 HF. What is the pH of the final solution? The value of K_a for HF is 6.8 x 10^-4.

Choose one answer.

	a. 4.65
	b. 2.20
	c. 7.00
	d. 3.45

Question 32

A solution contains 0.0128 g of HCl in 450. mL of solution. What is the pH of this solution at 25 °C?

Choose one answer.

	a. 1.00
	b. 7.00
	c. 3.10
	d. 10.89

Question 33

A solution contains 0.384 g of KOH in 250. mL of solution. What is the pH of this solution at 25 °C?

Choose one answer.

	a. 1.56
	b. 12.44
	c. 2.67
	d. 11.33

Question 34

An important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. The pH of blood is 7.44. What is the pH of blood, if 25% of the hydrogen phosphate is converted to dihydrogen phosphate? The value of K_a for H₂PO₄^- is 6.2 x 10^-2.

Choose one answer.

	a. 2.90
	b. 6.59
	c. 7.44
	d. 7.16

Question 35

At 10 °C, K_w = 2.9 x 10^-15. What is [OH^-] in neutral water at 10 °C?

Choose one answer.

	a. 4.44 x 10⁻⁶ M
	b. 1.00 x 10⁻⁷ M
	c. 1.70 x 10⁻⁷ M
	d. 5.39 x 10⁻⁸ M

Question 36

At 50 °C, K_w = 5.48 x 10^-14. What is [OH^-] in water of pH = 3 at 50 °C?

Choose one answer.

	a. 1.00 x 10⁻³ M
	b. 5.48 x 10⁻¹¹ M
	c. 5.48 x 10⁻⁷ M
	d. 2.74 x 10⁻⁷ M

Question 37

HC₂Cl₃O₂ is a stronger acid than HCHO₂. What is the direction of the equilibrium of the following reaction?
HC₂Cl₃O₂(aq) + CHO₂^-(aq) → C₂Cl₃O₂^-(aq) + HCHO₂(aq)

Choose one answer.

	a. The equilibrium lies to the left.
	b. The equilibrium lies to the right.
	c. The equilibrium is perfectly balanced left and right.
	d. This cannot be determined from the information given.

Question 38

H₃PO₄ is a stronger acid than NH₄⁺. What is the direction of the equilibrium of the following reaction?
NH₄⁺(aq) + H₂PO₄^-(aq) → NH₃(aq) + H₃PO₄(aq)

Choose one answer.

	a. The equilibrium lies to the left.
	b. The equilibrium lies to the right.
	c. The equilibrium is perfectly balanced left and right.
	d. This cannot be determined from the information given.

Question 39

The following solutions are mixed in equimolar portions. Will the resulting solution be acidic, basic, neutral, or is there not enough information given?
HCl(aq) + NaHCO₃(aq) → ?

Choose one answer.

	a. Acidic
	b. Basic
	c. Neutral
	d. This cannot be determined from the information given.

Question 40

What are the products of the following acid-base reaction?
HCl(aq) + NaOH(aq) → ?

Choose one answer.

	a. H₃O⁺(aq) + OH⁻(aq)
	b. Na⁺(aq) + Cl⁻(aq)
	c. H₂O(l) + NaCl(aq)
	d. No reaction takes place.

Question 41

What is a Brønsted-Lowry acid?

Choose one answer.

	a. A proton donor
	b. A proton acceptor
	c. An electron pair donor
	d. An electron pair acceptor

Question 42

What is a Lewis acid?

Choose one answer.

	a. A proton donor
	b. A proton acceptor
	c. An electron pair donor
	d. An electron pair acceptor

Question 43

What is a Lewis base?

Choose one answer.

	a. A proton donor
	b. A proton acceptor
	c. An electron pair acceptor
	d. An electron pair donor

Question 44

What is the pH of a buffer solution that is 0.15 M chloroacetic acid and 0.10 M sodium chloroacetate? The value of K_a for chloroacetic acid is 1.3 x 10^-3.

Choose one answer.

	a. 11.3
	b. 3.76
	c. 2.68
	d. 3.91

Question 45

What is the pH of the buffer solution that consists of 0.15 M pyridine and 0.10 M pyridinium bromide? The value of K_b for pyridine is 1.4 x 10⁹.

Choose one answer.

	a. 6.60
	b. 3.50
	c. 5.32
	d. 7.00

Question 46

What is the [OH^-] of a 5.43 x 10^-4 M solution of HNO₃ at 25 °C?

Choose one answer.

	a. 1.84 x 10⁻¹¹ M
	b. 5.43 x 10⁻¹⁰ M
	c. 5.43 x 10⁻⁴ M
	d. 3.67 x 10⁻⁸ M

Question 47

What will happen to the pH a solution of NH₃ by adding HCl?

Choose one answer.

	a. The pH will increase.
	b. The pH will decrease.
	c. The addition of HCl will not change the pH of the solution.
	d. There is not enough information given to determine this.

Question 48

Which of the following is an acid-base conjugate pair?

Choose one answer.

	a. HF and F⁻
	b. HNO₂ and NO₃⁻
	c. HClO and Cl⁻
	d. H₂CO₃ and CO₃²⁻

Question 49

Which of the following is NOT an acid-base conjugate pair?

Choose one answer.

	a. HCN and CN⁻
	b. HNO3 and NO3⁻
	c. HCl and ClO⁻
	d. NH4⁺ and NH3

Question 50

What is a Brønsted-Lowry base?

Choose one answer.

	a. A proton donor
	b. A proton acceptor
	c. A hydroxide donor
	d. An electron pair donor

Question 51

A particular voltaic cell operates on the following reaction.
Zn(s) + Cl₂(g) → Zn²⁺(aq) + 2 Cl^-(aq)
Given an emf of 0.853 V, calculate the maximum electrical work generated when 20.0 g of zinc metal is consumed.

Choose one answer.

	a. -8.23 x 10⁴ J
	b. -1.65 x 10⁵ J
	c. -5.03 x 10⁴ J
	d. -2.51 x 10⁴ J

Question 52

A voltaic cell has the following reaction.
Zn(s) + 2 Fe³⁺(aq) → 2 Fe²⁺(aq) + Zn²⁺(aq) E° = 0.72 V
What is the maximum electrical work that can be obtained from this cell per mole of iron (III) ion?

Choose one answer.

	a. +69 kJ
	b. -140 kJ
	c. -69 kJ
	d. 1.4 J

Question 53

Cadmium reacts spontaneously with copper(II) ion.
Cd(s) + Cu²⁺(aq) → Cd²⁺(aq) + Cu(s)
What are the half reactions for this reaction?

Choose one answer.

	a. Cd(s) + 2e⁻ → Cd²⁺(aq) and Cu²⁺(aq) + 2e⁻ → Cu(s)
	b. Cd(s) → Cd²⁺(aq) + 2e⁻ and Cu²⁺(aq) → Cu(s) + 2e⁻
	c. Cd(s) → Cd²⁺(aq) + e⁻ and Cu²⁺(aq) + e⁻ → Cu(s)
	d. Cd(s) → Cd²⁺(aq) + 2e⁻ and Cu²⁺(aq) + 2e⁻ → Cu(s)

Question 54

Calculate the emf for a cell operating with the following reaction:
Cr₂O₇^2-(aq) + 6 I^-(aq) + 14 H⁺(aq) → 2 Cr³⁺(aq) + 3 I₂(s) + 7 H₂O(l),
where [Cr₂O₇^2-] = 0.020 M, [I^-] = 0.015 M, [Cr³⁺] = 0.20 M and [H⁺] = 0.50 M, using the following standard reduction potentials:
Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- → 2 Cr³⁺(aq) + 7 H₂O(l) E° = +1.33 V
I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V

Choose one answer.

	a. +1.87 V
	b. -1.87 V
	c. +0.79 V
	d. +0.64 V

Question 55

Calculate the equilibrium constant K for the following reaction at 25 °C.
2 Fe³⁺(aq) + Cu(s) → 2 Fe²⁺(aq) + Cu²⁺(aq) E° = +0.43 V

Choose one answer.

	a. 7.26
	b. 0.43
	c. 3.4 x 10¹⁴
	d. 1.7 x 10⁷

Question 56

Calculate ΔG° for the following reaction at 25 °C.
3 Cu(s) + 2 NO₃^-(aq) + 8 H⁺(aq) → 3 Cu²⁺(aq) + 2 NO(g) + 4 H₂O(l) E° = +0.62 V

Choose one answer.

	a. -3.6 x 10⁵ J
	b. -6.0 x 10⁴ J
	c. 3.6 x 10⁵ J
	d. 1.2 x 10⁵ J

Question 57

Fill in the blank. When a piece of iron is left outside, it will rust. In this situation, the iron atoms are _______________.

Choose one answer.

	a. Losing electrons
	b. Gaining electrons
	c. Staying neutral
	d. Combining with nitrogen gas from the air

Question 58

Given the following two half reactions,
Cd²⁺(aq) + 2e^- → Cd(s) E° = -0.40 V
2 Ag⁺(aq) + 2e^- → 2 Ag(s) E° = 0.80 V
determine E° and the spontaneity of the following reaction:
2 Ag⁺(aq) + Cd(s) → 2 Ag(s) + Cd²⁺(aq)

Choose one answer.

	a. +0.40 V and not spontaneous
	b. +1.20 V and spontaneous
	c. +1.20 V and not spontaneous
	d. -0.40 V and spontaneous

Question 59

Given the two following half reactions,
Cl₂(g) + 2e- → 2 Cl^-(aq) E° = +1.36 V
I₂(g) + 2e- → 2 I^-(s) E° = +0.54 V
calculate ΔG° for the following reaction:
2 I-(aq) + Cl₂(g) → 2 Cl-(aq) + I₂(s).

Choose one answer.

	a. -1.6 kJ
	b. -7.9 x 10⁴ J
	c. -1.6 x 10⁵ J
	d. -79 kJ

Question 60

Given the two following half reactions,
Sn²⁺(aq) + 2e^- → Sn(s) E° = -0.14 V
Cu²⁺(aq) + 2e^- → Cu(s) E° = +0.34 V
calculate the standard emf for the following reaction:
Sn(s) + Cu²⁺(aq) → Sn²⁺(aq) + Cu(s).

Choose one answer.

	a. 0.96 V
	b. -0.48 V
	c. +0.20 V
	d. 0.48 V

Question 61

Given the two following half reactions,
Cr³⁺(aq) + 3e^- → Cr(s) E° = -0.74 V
Hg2²⁺(aq) + 2e^- → Hg(l) E° = +0.80 V
calculate the standard emf for the following cell:
Cr | Cr³⁺|| Hg2²⁺| Hg

Choose one answer.

	a. -0.06 V
	b. -1.54 V
	c. +1.54 V
	d. +0.06 V

Question 62

How many coulombs of charge are required to form 1.00 pound of Al(s) from an Al³⁺ salt?

Choose one answer.

	a. 4.87 x 10⁶
	b. 50.5
	c. 1.62 x 10⁶
	d. 454

Question 63

If we wish to convert 1.00 g of Au³⁺(aq) ion into Au(s) in a "gold-plating" process, how long must we electrolyze a solution if the current passing through the circuit is 2.00 amps?

Choose one answer.

	a. 245 sec
	b. 0.50 sec
	c. 0.015 sec
	d. 735 sec

Question 64

Of the following four reactions, how many are oxidation-reduction reactions?
NaOH + HCl → NaCl + H₂O
Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂
Mg(OH)₂ → MgO + H₂O
N₂ + 3 H₂ → 2 NH₃

Choose one answer.

	a. 0
	b. 1
	c. 2
	d. 3

Question 65

The voltaic cell Cd | Cd²⁺|| Ni²⁺| Ni has an E° of 0.170 V. If the standard reduction potential of Ni²⁺/Ni is E° = -0.23 V, what is the standard reduction potential for Cd²⁺/Cd?

Choose one answer.

	a. +0.06 V
	b. -0.06 V
	c. -0.40 V
	d. +0.40 V

Question 66

The voltaic cell Cd | Cd²⁺|| Ni²⁺ (1.0M)| Ni has an electromotive force of 0.240 V at 25 °C. What is the concentration of cadmium ion? (Please note that E° = 0.170 V.)

Choose one answer.

	a. 0.06 M
	b. 0.04 M
	c. 0.004 M
	d. 1.0 M

Question 67

What are the half reactions for the electrolysis of LiCl(l)?

Choose one answer.

	a. Cathode: Li⁺(l) → Li(l) + e⁻ and Anode: 2 Cl⁻(l) → Cl₂(g) + 2 e⁻
	b. Cathode: Li⁺(l) → Li(l) + e⁻ and Anode: 2 Cl⁻(l) + 2 e⁻ → Cl₂(g)
	c. Cathode: 2 Cl⁻(l) → Cl₂(g) + 2 e⁻ and Anode: Li⁺(l) + e⁻ → Li(l)
	d. Cathode: Li⁺(l) + e⁻ → Li(l) and Anode: 2 Cl⁻(l) → Cl₂(g) + 2 e⁻

Question 68

What is the cell notation for a voltaic cell with the following equation?
Pb²⁺(aq) + Cd(s) → Pb(s) + Cd²⁺(aq)

Choose one answer.

	a. Pb \| Pb²⁺\|\| Cd²⁺\| Cd
	b. Pb²⁺ \| Pb \|\| Cd \| Cd²⁺
	c. Cd \| Cd²⁺\|\| Pb²⁺ \| Pb
	d. Cd \| Pb²⁺\|\| Pb \| Cd²⁺

Question 69

What is the correct balanced equation for the following oxidation-reduction reaction?
Cr₂O₇^2- + C₂O₄^2- → Cr³⁺ + CO₂

Choose one answer.

	a. Cr₂O₇²⁻ + 3 C₂O₄²⁻ → 2 Cr³⁺ + 6 CO₂
	b. 28 H⁺ + 2 Cr₂O₇²⁻ + 3 C₂O₄²⁻ → 4 Cr³⁺ + 6 CO₂ + 14 H₂O
	c. 14 H⁺ + Cr₂O₇²⁻ + C₂O₄²⁻ → Cr³⁺ + 2 CO₂ + 7 H₂O
	d. 14 H⁺ + Cr₂O₇²⁻ + 3 C₂O₄²⁻ → 2 Cr³⁺ + 6 CO₂ + 7 H₂O

Question 70

What is the overall cell reaction for the following voltaic cell?
Fe | Fe²⁺|| Ag⁺| Ag

Choose one answer.

	a. Ag⁺(aq) + Fe(s) → Ag(s) + Fe²⁺(aq)
	b. 2 Ag⁺(aq) + Fe(s) → 2 Ag(s) + Fe²⁺(aq)
	c. 2 Ag(s) + Fe²⁺(aq) → 2 Ag⁺(aq) + Fe(s)
	d. Fe(s) + Fe²⁺(aq) → Ag⁺(aq) + Ag(s)

Question 71

Fill in the blank. In the reaction Cu(s) + 4HNO₃(aq) → Cu(NO₃)₂(aq) + 2NO₂(g) + 2H₂O(l), copper is __________.

Choose one answer.

	a. Reduced
	b. Electrolyzed
	c. Synthesized
	d. Oxidized

Question 72

Beta decay of the nucleus of

produces which of the following nuclide?

Choose one answer.

	a. Ra
	b. Ac
	c. Pa
	d. U

Question 73

Sodium is a very reactive metal. Its ion is found in table salt. While non-radioactive sodium is abundant, there exists a radioactive isotope of sodium, Sodium-24. Its half life is 15 hours. If after 60 hours, about 6 grams remain, then what was the original mass of the sodium-24 sample?

Choose one answer.

	a. 50 g
	b. 40 g
	c. 100 g
	d. 60 g

Question 74

Technetium-99 has a half-life of 6.0 hrs. What fraction of Technetium-99 in the sample will remain undecayed after 36 hours?

Choose one answer.

	a. 1/8
	b. 1/64
	c. 1/32
	d. 1/16

Question 75

The half life of Colbalt-60 is 5.2 years. What happens to an aliquot of cobalt-60 after 5.2 years?

Choose one answer.

	a. The concentration decreases by half.
	b. The cobalt changes to cobalt-30.
	c. The cobalt-60 atom breaks in half.
	d. The concentration doubles.

Question 76

What are beta particles?

Choose one answer.

	a. Highly active electrons diffused from radioactive nuclei
	b. Less active protons diffused from standard nuclei
	c. Highly active neutrons in radioactive nuclei
	d. X-rays that allow radioactive nuclei's to be viewed

Question 77

What is the amount of radioactive sample that has NOT decayed after three-half lives have elapsed?

Choose one answer.

	a. 1/3 the original amount
	b. 1/9 the original amount
	c. ¼ the original amount
	d. 1/8 the original amount

Question 78

What is the correct alternate notation for gold-197?

Choose one answer.

	a.
	b.
	c.
	d.

Question 79

What is the half-life of a radioactive nuclide?

Choose one answer.

	a. The period of time in which 25% of the original number of atoms undergoes radioactive decay
	b. The time at which the isotope becomes non radioactive
	c. The period of time in which 50% of the original number of atoms undergoes radioactive
	d. The period of time it takes to reduce radioactivity by 100%

Question 80

Which nuclide contains 11 protons, 11 electrons, and 14 neutrons?

Choose one answer.

	a. Silicon-11
	b. Silicon-14
	c. Sodium-11
	d. Sodium-25

Question 81

Which of the following best describes how the atomic number changes when a nucleus captures an electron?

Choose one answer.

	a. It will increase by one.
	b. It will decrease by one.
	c. It will not change, because the electron has such a small mass.
	d. It will increase by two.

Question 82

Which of the following elements is the daughter nuclide for the alpha decay of polonium-212?

Choose one answer.

	a. Lead-208
	b. Lead-216
	c. Radon-208
	d. Radon-216

Question 83

Which type of radiation has the most penetrating ability?

Choose one answer.

	a. An alpha particle
	b. A beta particle
	c. A gamma ray
	d. A neutron

Question 84

Which of the following processes is NOT an example of a spontaneous radioactive process?

Choose one answer.

	a. Alpha-decay
	b. Auto ionization
	c. Positron production
	d. Beta-decay

Question 85

Fill in the blank. CH₃CH₂CH₂C≡CCH₂CH₂Cl is named __________.

Choose one answer.

	a. 7-chloro-4-heptyne
	b. 5-chloro-2-heptene
	c. 1-acetylenenyl-3-chloropropane
	d. 1-chloro-3-heptyne

Question 86

How many structural isomers does butane have?

Choose one answer.

	a. 1
	b. 2
	c. 3
	d. 4

Question 87

How many types of alkyl groups can arise from propane?

Choose one answer.

	a. 0
	b. 1
	c. 2
	d. 3

Question 88

Kira was doing some organic chemistry nomenclature problem. She gave a molecule the following name: 2-Methyl-4-methylhexane. While one can correctly draw the molecule from the name she gave, the name violates the IUPAC rules. What is the IUPAC name of the molecule?

Choose one answer.

	a. 2,4-dimethylhexane
	b. 3-Methyl-5-methylhexane
	c. 3,5-dimethylhexane
	d. 1-isopropyl-2-methylbutane

Question 89

Nylon is an example of which of the following?

Choose one answer.

	a. Copolymer
	b. Homopolymer
	c. Dimer
	d. None of the above

Question 90

Teflon is an example of which of the following?

Choose one answer.

	a. Copolymer
	b. Homopolymer
	c. Dimer
	d. None of the above

Question 91

The name methanal is the IUPAC name for which of the following?

Choose one answer.

	a. Acetone
	b. Formaldehyde
	c. Water
	d. Rubbing alcohol

Question 92

What is the general name given to hydrocarbons with double bonds?

Choose one answer.

	a. Alkenes
	b. Alkynes
	c. Alkanes
	d. Aromatic hydrocarbons

Question 93

What is the name of the following molecule?
CH_3-(CH₂)₇-CH₃

Choose one answer.

	a. Heptane
	b. Hexane
	c. Octane
	d. Nonane

Question 94

Which of the following accurately provides the generalized molecular formulas for alkanes and alkenes respectively?

Choose one answer.

	a. C_nH_2n+2 and C_nH_2n
	b. C_nH_2n and C_nH_2n+2
	c. C_nH_2n+2 and C_nH_2n-2
	d. C_nH_2n and C_nH_2n+1

Question 95

Which of the following CANNOT form alkenes?

Choose one answer.

	a. Methane
	b. Ethane
	c. Propane
	d. All of the above

Question 96

Which of the following has the greatest number of C-O bonds?

Choose one answer.

	a. Ketone
	b. Ester
	c. Alcohol
	d. Amine

Question 97

Which of the following has the least number of C-O bonds?

Choose one answer.

	a. Ketone
	b. Alcohol
	c. Ether
	d. Ester

Question 98

Which of the following is known as rubbing alcohol?

Choose one answer.

	a. Methanol
	b. Ethanol
	c. Propanol
	d. Isopropanol

Question 99

Which of the following is known as wood alcohol?

Choose one answer.

	a. Methanol
	b. Ethanol
	c. Propanol
	d. Isopropanol

Question 100

In a triple bond, how many electrons are shared?

Choose one answer.

	a. 3
	b. 4
	c. 5
	d. 6